Preparation of Copper(I) Chloride Reactions: 1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2)...

Preparation of Copper(I) Chloride

Reactions:

1) Cu(S) + 4HNO₃(aq) -> Cu(NO₃)₂(aq) + 2NO₂(g) + 2H₂O(l)

2) 2HNO₃(aq) + Na₂CO₃(s) -> H₂O(l) + CO₂(g) + 2NaNO₃(aq)

3)Cu(NO₃)2(aq) + Na₂CO₃(s) -> CuCO₃(s) + 2NANO3(aq)

4)CuCO_3(s) + 2HCL(aq) -> CuCl_2(aq) + H₂O_(l) + CO_2(g)

5)CuCl₂(aq) + Cu(s) -> 2CuCl(s)

Report:

Weight of Copper: 1.004g

Volume of Added Nitric Acid: 4.9mL

Total weight of added Sodium Carbonate: 3.841g

Weight of watch glass and filter paper: 51.740g

Weight of watch glass, filter paper, and CuCl Precipitate: 53.513g

Experimental Yield of CuCl: 1.775g

Theoretical Yield of CuCl: 3.55g

Percent Yield of CuCl: 50%

Could we use HCl to dissolve the copper metal instead of nitric acid in the first reaction? Please explain.

Solutions

Expert Solution

NO.

When you are using Hydrochloric Acid (aka: HCl), it will "attack" nearly anything above hydrogen, including, Lead, Aluminum, Magnesium, Tin, Zinc, etc. (Lead is a bit of a challenge for HCl because Lead Chloride is insoluble, and can form a protective coat that stops the reaction from occurring. It does actually react on the surface and if you add some heat to the reaction, it can push it even further.) But, as Copper is below Hydrogen, it is not attacked by HCl...

With Nitric Acid (aka: HNO3), in dilute form, the reaction is the same as with HCl... However, if you are using concentrated HNO3, the nitrate portion of the acid IS able to attack the Copper... This, because the nitrate is a powerful oxidizing agent when in high concentration. The nitrate portion is reduced to NO2 gas and the metal is oxidized. This reaction allows concentrated nitric acid to also attack metals that are "below" hydrogen (to some extent). Mercury, copper, and silver are all readily attacked by this reaction...

queen_honey_blossom answered 1 year ago

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